The compound(s) with two lone pairs of electron on the central atom is (are)

Options

A. `BrF_(5)`
B. `ClF_(3)`
C. `XeF_(4)`
D. `SF_(4).`

Explanation

To determine the compounds with two lone pairs of electrons on the central atom, we can analyze the molecular structures of various compounds. Here’s a step-by-step solution:

### Step 1: Identify the central atom and its valence electrons
- The first step is to identify the central atom in the compound and count its valence electrons. For example, in ClF3, the central atom is chlorine (Cl), which has 7 valence electrons.

### Step 2: Draw the Lewis structure
- For ClF3, we draw the Lewis structure. Chlorine will form three bonds with three fluorine atoms, using 3 of its valence electrons. This leaves 4 electrons (2 lone pairs) on the chlorine atom.

### Step 3: Analyze the geometry
- The geometry of ClF3 is T-shaped due to the presence of two lone pairs and three bonding pairs. This confirms that ClF3 has two lone pairs on the central atom.

### Step 4: Check other compounds
- Next, we analyze XeF4 (xenon tetrafluoride). Xenon has 8 valence electrons. It forms four bonds with four fluorine atoms, using 4 electrons, which leaves 4 electrons (2 lone pairs) on the xenon atom.

### Step 5: Confirm the geometry of XeF4
- The geometry of XeF4 is square planar, which also confirms the presence of two lone pairs on the central atom.

### Step 6: Review other compounds
- For SF4 (sulfur tetrafluoride), sulfur has 6 valence electrons and forms four bonds with fluorine atoms. This leaves 1 lone pair on the sulfur atom, which does not meet the criteria of having two lone pairs.

### Conclusion
- The compounds with two lone pairs of electrons on the central atom are ClF3 and XeF4.

### Final Answer
The compounds with two lone pairs of electrons on the central atom are:
1. ClF3 (Chlorine trifluoride)
2. XeF4 (Xenon tetrafluoride)

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